2AB Chemistry

• describe the characteristics of homogeneous and heterogeneous mixtures
• distinguish between pure substances, homogeneous mixtures and heterogeneous mixtures.

• use the Kinetic Theory of Matter to explain
  • relationship between heat and temperature
  • change of phase
  • vapour pressure and factors that affect vapour pressure
  • effect on gases of changes in pressure, temperature and volume
  • the characteristics of gases
• predict the effect on gases of changes in pressure, temperature and volume (qualitative only)
• explain the boiling point of a liquid.

• identify, explain and give examples of saturated, unsaturated and supersaturated solutions
• apply solubility rules to predict if a precipitate will form when two dilute ionic solutions are mixed (see data sheet)
• use the colour of ions (see data sheet) to identify reactants and the products in chemical processes
• explain the effect of concentration on vapour pressure, melting point and boiling point of a solution
• describe the characteristics and give examples of strong, weak and non-electrolytes
• explain the differences between concentrated and dilute solutions of strong and weak electrolytes.

• describe and give examples of solutions and their uses in and around the home
• explain concentration units used in household mixtures (g 100g-1,mL L-1, g mL-1, percentage composition)
• calculate concentration (mixtures (g 100g-1,mL L-1, g mL-1,)

• compare the relative charge and relative masses of protons, neutrons and electrons
• identify elements using their atomic number (Z)
• explain isotopes using their atomic number (Z) and mass number (A)
• use the energy level or shell model of electron structure to write the electron configurations for the first twenty elements (Na 2, 8, 1)
• explain the relationship between position on the Periodic Table and number of valence electrons of elements in groups 1, 2 and 13–18
• explain the relationship between the number of valence electrons and chemical properties of elements in groups 1, 2 and 13–18
• explain the formation of positive and negative ions for elements in groups 1, 2 and 13–18.

• describe and explain the formation and characteristics of:
  • ionic bonds and ionic substances
  • metallic bonds and metallic substances
  • covalent bonds
  • covalent network and molecular substances
• describe and explain the relationships between properties and structures of ionic, metallic, covalent network and covalent molecular substances
• draw representations of molecular and ionic substances using electron dot (octet only) or Lewis structure diagrams.

• describe the relationships between properties and uses of ionic, metallic, covalent network and covalent molecular substances found in and around the home

• use the Law of Conservation of Energy to explain endothermic and exothermic reactions
• apply the concepts of system and surroundings to energy transfer
• explain enthalpy (H) in terms of stored chemical energy
• explain endothermic and exothermic reactions in terms of bond breaking and bond making
  • interpret and explain enthalpy diagrams and equations that include the heat lost or gained (ΔH).
  
  
  Applied chemistry
  • describe and explain common examples of endothermic and exothermic reactions or processes in and around the home e.g. combustion, hot packs, change of phase
  Reaction rates
  • describe the rate of a reaction in terms of rate of change of a measurable quantity with time
  • identify and apply the factors affecting rates of reaction:
    • concentration
    • catalysts
    • temperature
    • state of sub-division
    • apply the collision theory to explain the factors affecting rates of reaction
    • draw and interpret energy profile diagrams to show the transition state, activation energy, uncatalysed and catalysed pathways and the heat of reaction
    • explain the relationship between collision theory, kinetic energy distribution graphs and the rate of a reaction.
  
  
  Applied chemistry
  • describe and explain examples where rates of reaction have been altered in and around the home
  • investigate real world problems in a laboratory setting with appropriate teacher direction, considering:
    • sources of uncertainty in experimental measurements
  selection of the appropriate units of measurement of quantities such as volume and time.

• write and interpret formulae of elements and compounds
• describe, write equations and predict observations for precipitation reactions
• write equations that show only the species involved in the reaction

• perform simple gravimetric calculations:
• molar mass
  • mole to mole
  • mass to mole
  • mass to mass
    • calculate concentration (mixtures (g 100g-1,mL L-1, g mL-1,)
    • percentage composition
  
  Applied chemistry
  • write the chemical formulae for molecular compounds based on the number of atoms of each element present as inferred from the systematic names
  • write the molecular formulae of commonly encountered molecules that have non-systematic names
  • explain conservation of mass, atoms and charge during a chemical reaction

Content - 2B Chemistry

• describe, explain and apply an understanding of the Arrhenius and Brønsted-Lowry models of acids and bases
• describe and explain the difference between strong acids, including HCl, H2SO4, HNO3 and weak acids including CH3COOH and H3PO4
• identify acids by:
  • indicator colour
  • pH scale value
  • reaction with:
    • metal carbonates and hydrogen carbonates
    • metals such as magnesium and iron
    • metal oxides
    • metal hydroxides
• describe and explain the difference between strong bases, including group 1 and group 2 hydroxides and weak bases including NH3 and Na2CO3
• identify bases by:
  • indicator colour
  • pH scale value
  • reaction with:
    • acids
    • ammonium salts
• write equations for the reactions of acids showing only the species involved, using state symbols where appropriate
• describe, write equations and predict observations for the following reactions:
  • acid-base
  • acid-carbonate
  • acid-metal
• write equations for the successive ionisation of polyprotic acids
• qualitatively apply the pH scale
• describe properties and reactions of non-metal and metal oxides e.g. reaction of SO2 with water
• perform stoichiometric problems that interrelate mass, molar mass, number of moles of solute, and concentration and volume of solution
• mass to volume (gases at STP)
• limiting reagent

• explain oxidation and reduction as an electron transfer process
• calculate oxidation numbers
• identify and name oxidants and reductants in equations
• identify oxidation-reduction reactions using oxidation numbers
• describe, write equations for and interpret observations for:
  • metal displacement reactions
  • halogen displacement reactions
• write balanced simple redox equations (metal/metal ion, metal/hydrogen ion and halogen/halide ion)
• describe and explain how an electric current is conducted in an electrolytic cell
• describe and explain the following during the operation of an electrolytic cell:
  • anode processes
  • cathode processes
  • role of the electrolyte
  • direction of ion migration
  • direction of electron flow in external circuit
  • electrode product prediction for molten metal halides only
  • predict and name the electrode products for the electrolysis of molten metal halides only

• describe the bonding capacity of carbon
• explain the diversity of carbon based compounds
• Alkanes:
  • name and draw straight and simple branched to C8
    • observations and equations for:
      • substitution reactions
      • combustion reactions
    • draw and name structural isomers
• Alkenes:
  • name and draw straight and simple branched to C8 (only one double bond per structure)
    • write observations and equations for:
      • addition reactions with halogens and hydrogen
      • combustion reactions
  • draw and name structural and geometric isomers
  • Cycloalkanes and cycloalkenes:
    • draw and name simple structures to C8
    • write observations and equations for:
      • substitution and combustion reactions for cycloalkanes
      • addition and combustion reactions for cycloalkenes
    • Benzene:
      • explain the unique structure and reactivity of benzene
      • write equations for:
        • catalysed substitution reactions with halogens
        • combustion reactions
    Applied chemistry
    • describe and explain the sources and uses of hydrocarbons e.g. fuels
    • determine molecular formulae (organic or inorganic) from empirical formula and molar mass
    empirical formula calculations using percentage composition, mass composition and combustion data

• Mixtures
• Solutions

• Kinetic theory

• Atoms and isotopes

• Atomic structure and the periodic table

• Bonding

• Uses, properties and structure

• Elements and compounds

• Molar mass

• Moles, particles and mass

• Interpretation of formulae

• Percentage composition

• Ionic equations

• Stoichiometry and gas volumes

• Solution concentrations

• Solution of acids and bases

• Acid and base reaction stoichiometry

• Empirical formulae

• Limiting reagents

• Gas volumes

• Stoichiometry

• Reacting masses and gaseous and solution volumes

• Equations and observations

• Oxidation number (ON)

• Balancing half equations

• Balancing overall redox equations

• Naming and drawing hydrocarbons

• Reactions of hydrocarbons

• Calculations involving hydrocarbons